SOLANO COLLEGE



SOLANO COLLEGE - CHEMISTRY 160 (Section 6365), SPRING 2006

|LECTURE (Vasfi Basaran): |W 6:00 PM - 8:50 PM (VJFKL) |

|LAB: |Sat 9:00 AM - 11:50 AM (Room 303) |

|OFFICE : |TBA |

| |Phone: 707.864.7000 x5258 |

| |Email: vasifi.basaran@solano.edu |

|OFFICE HOURS: |Before or after lecture / lab |

| |or by appointment |

Welcome to Chemistry 160, a four unit general chemistry course. This is an introductory course covering the principles of inorganic chemistry. It includes 3 hours of lecture and 3 hours of lab each week. Prerequisite: A grade of “C” or better in Math 104 or two years of high school algebra with a grade of “C” or better.

Required Materials:

Text: Stoker, INTRODUCTION TO CHEMICAL PRINCIPLES 8nd ed, Pearson/Prentice Hall, 2005.

Lab Text: Weiner, CHEMICAL PRINCIPLES: A Laboratory Approach, 6TH Edition, Harcourt College Publishers 2004

Chemtutor CD (available in the back of the bookstore)

Calculator

Safety glasses or goggles

Disposable lab gloves

Course Content:

Topics (units) include composition of matter, atomic theory and the periodic table of the elements; naming compounds; writing formulas; balancing chemical equations; recognizing, naming and writing chemical reactions; solution chemistry; stoichiometry; acids and bases. A detailed list is attached which outlines the topics to be covered in each unit. The course will include problem solving and hands-on laboratory experiments in each of these areas. This course will prepare you to take Chem 1 or Chem 10 as you continue your studies here at Solano.

Lab work will provide hands-on practice of the subjects learned in lecture. There will also be an opportunity in lab to use computer tutorials to reinforce learning of the subject matter. The first hour of each lab session will be either lecture, discussion or computer work. The second and third hour will be hands-on lab work.

Disclaimer: This syllabus is subject to change at any time. However, changes will be announced in advance!

Evaluation and Grading:

Quizzes and tests will be announced in advance. Some quizzes are take-home quizzes. The lowest quiz and the lowest exam grade will be dropped. There will be no make-up quizzes or exams. Homework will not be collected or graded. However, you must do the recommended practice problems to succeed in this course. There will be worksheets for in-class group work and for completion at home. Lab work is described in a later section of this syllabus.

The following table shows the distribution of points for evaluating your grade in this course. Also, point totals may change as the number of exams and assignments change to meet student’s needs through the semester.

| |Course Grade |

|Quizzes (~8 – drop one) 150 (15%) |A ≥ 90% (≥ 900 pts) |

|Unit Exams (4 – drop one) 300 (30%) |B ≥ 80% (≥ 800 pts) |

|Final Exam 300 (30%) |C ≥ 65% (≥ 650 pts) |

|Lab 250 (25%) |D ≥ 50% (≥ 500 pts) |

|------------------------- --------------- |F < 50% (< 500 pts) |

|1000 (100%) | |

|Quizzes, tests and lab reports will be given a point grade, not a letter grade. Only your final course grade will be given a |

|letter grade. |

I will do what I can to ensure your success in understanding and learning chemistry. I will present organized lectures with an occasional demonstration, organize and explain the laboratory experiments and their relevance to the lecture material. I will return your quizzes and exams promptly so you will know how you are doing in the course. I will be available to help you in any way I can.

YOUR PART is to attend all lectures and labs, read the text, do the recommended homework, fill out lab reports, use the computer to study and ask questions in lecture and lab. On average, you will need to do 2 hours of homework for every hour in lecture and about one hour for every 3 hours in lab (7 hours of work outside of class each week). Homework includes reading the text and lab book material before class, re-reading and re-writing lecture notes and text book material for complete understanding after class, doing the assigned problems, and writing lab reports. It is very helpful to meet with a study group once a week. Working together and teaching each other in a study group is a proven way to learn a new subject.

You must keep up. Chemistry is a difficult subject that requires consistent studying. Don’t try to “catch up” just before the exam. If you need help, talk to me before or after class or by appointment. If you need more help, you can also arrange for a tutor through the on-campus-tutoring center.

Even though you do all these things, you may find circumstances dictate withdrawing. It is your responsibility to file paperwork on time and withdraw from class and lab. If you don’t, you may end up with an F in the course.

Important Dates:

Fri, January 27 Last day to register or add classes & last day to drop with full refund

Thurs, February 16 Last day drop a class

Last day to file for credit/no credit option

Fri, April 7 Last day to drop classes with a “W” grade

Sat, May 20 Final Exam

LECTURE SCHEDULE and PRACTICE PROBLEMS

|Week / Week|Chapter.section / Topic(s) |Practice Problems |

|of | | |

|1 / | |Ch 1.1 – 1.4 Introduction / Scientific method + periodic table 1st 36 elements and … |Do all corresponding odd numbered |

|1/16 | |Ch 2.1 – 2.8 Measurements, significant figures and scientific notation |problems |

|2 / | |(QUIZ #1) | |

|1/23 | |Ch 3.1 – 3.5 Metric Units + selected positive and negative ions | |

| | |Ch 3.6 – 3.11 Conversion factors and dimensional analysis, density, temperature scales, percentage and percent error. | |

|3 / | |(QUIZ #2) | |

|1/30 | |Ch 4.1 – 4.9 Classification of matter | |

| | |Ch 5.1 – 5.8 Atomic theory + selected polyatomic ions | |

|4 / | |EXAM #1 (Chp 1, 2, 3, 4) | |

|2/6 | |Chp 6.1 – 6.2 Periodic table | |

|5 / | |(QUIZ #3) | |

|2/13 | |Chp 6.3 – 6.12 Quantum model of the atom | |

| | |Chp 7.1 – 7.9 Ionic Bonding | |

|6 / | |(QUIZ #4) | |

|2/20 | |Chp 7.10 – 7.15 Covalent bonding | |

| | |Chp 7.16 – 7.20 Structure and Shape | |

|7 / | |(QUIZ #5) | |

|2/27 | |Chp 8.1 – 8.3 Nomenclature | |

| | |Chp 8.4 – 8.7 | |

|8 / | |EXAM #2 (Chp 5, 6, 7, 8) | |

|3/6 | |Chp 9.1 – 9.4 Chemical Formulas and percent composition | |

| | |Chp 9.5 – 9.8, 9.11 - 9.12 Moles, Avogadros number, molar mass and percent purity | |

|9 / | |(QUIZ #6) | |

|3/13 | |Chp 9.10, 9.13 – 9.15 Empirical and molecular formulas | |

| | |Chp 10.1 – 10.4 Writing and balancing chemical equations | |

| | |Chp 10.5 types of reactions | |

|10 / | |(QUIZ #7) | |

|3/20 | |Chp 10.6 – 10.10 Mass calculations using chemical equations | |

| | |Chp 11.1 – 11.7 Gases, Liquids, Solids, kinetic molecular theory | |

|11 / | |EXAM #3 (Chp.9,10) | |

|10/31 | |Chp 11.8 Energy changes in phase transformations | |

|12 / | |(QUIZ #8) | |

|3/27 | |Chp 11.13 – 11.16 Properties of liquids, intermolecular forces, water | |

| | |Chp 13.1 - 13.4 Solutions | |

|13 / | |(QUIZ #9) | |

|4/3 | |Chp 13.5 – 13.8 Solution concentration (mass percent, ppm and ppb, molarity) | |

| | |Chp 13.10 – 13.11 Solution stoichiometry | |

|14 / | |Spring Vacation | |

|4/10 | | | |

|15 / | |(QUIZ #10) | |

|4/17 | |Chp 14.1 – 14.5 Acids and bases | |

| | |Chp 14.6 – 14.10 Electrolyte and non-electrolyte solutions and net ionic equations | |

|16 / | |EXAM #4 (Chp 11, 13, 14) | |

|4/24 | |Chp 14.11 – 14.12 water equilibrium and pH | |

|17 / | |TBA | |

|5/1 | | | |

| | |Sat. May 20 FINAL EXAM |Comprehensive final |

WHAT YOU NEED TO KNOW

UNIT 1

Chp 1 – INTRODUCTION

• Definition of Chemistry. Why is it called the central science?

• (1.4) Scientific Method

• Natural laws: LAW OF CONSERVATION OF MASS - Mass is constant in a chemical reaction; it is neither created nor destroyed.

Chp 2 – MEASUREMENT

• (2.1 – 2.3) Measurement, exact and inexact numbers, accuracy, precision and error

• (2.4 – 2.6) Significant figures and rounding

• (2.7 – 2.8) Scientific (exponential notation)

Chp 3 – UNIT SYSTEMS & DIMENSIONAL ANALYSIS

• (3.1 – 3.5) Metric units

← Metric prefixes required to know: pico, nano, micro, milli, centi, kilo, mega, giga

• Conversions to memorize

1 kg = 1000 g 1 cm3 = 1 mL 1 m = 100 cm 1 L = 1000 mL

• (3.6 - 3.7) Conversion factors and dimensional analysis

• (3.8 – 3.11) Density and specific gravity, percentage and percent error, temperature scales ( know ( o F – 32 = 1.8 x o C)

Chp 4 – MATTER

Definition of

• (4.1) Matter

• (4.2) States of matter

• Macroscopic, microscopic and particulate matter

• (4.3 – 4.4) Physical vs. chemical properties and changes

• (4.5) Pure substances and mixtures

• (4.6) Homogeneous and heterogeneous matter

• (4.7 – 4.9) Elements and compounds (names and symbols)

UNIT 2

Chp 5 – ATOMIC STRUCTURE

• (5.1) Daltons Atomic Theory

• (5.2 – 5.4) Elements, Molecules, Formulas

• (5.5, 5.9) Subatomic particles – electron, proton, neutron (know charge and relative size)

• (5.9) The nuclear model of the atom (Rutherford’s experiment)

• (5.6 – 5.7) Atomic number and mass number and isotopes

• (5.8) Calculation of atomic mass

Chp 6 – ELECTRON STUCTURE OF THE ATOM

• (6.1 – 6.2) Periodic Table (Mendeleev)

• (6.3 - 6.4) Bohr Model of the atom (quantized energy levels)

• (6.5 – 6.6) Quantum model of the atom (energy sublevels and orbitals)

• (6.7 – 6.8) Electron configuration and orbital diagrams (Aufbau principle and aufbau diagram)

• (6.9 – 6.10) Valence electrons and the periodic law

• (6.11- - 6.12) Classification of elements and trends in the periodic table (atomic size, ionization energy, metallic character)

Chp 7 – CHEMICAL BONDING & MOLECULAR SHAPE

• (7.1) Know the difference between ionic and covalent bonds

• (7.2 – 7.3) Valence electrons, Lewis symbols and the Octet Rule

• (7.4 – 7.5) Know formation of monatomic ions (cations and anions) and the electron configuration of ions

• (7.6 – 7.9) Formation, formulas, structure of ionic compounds

• (7.10 – 7.15) Covalent bonds, Lewis structures, multiple bonds, coordinate covalent bonds, resonance structures.

• (7.16) Know how to draw Lewis structures of covalent compounds

• (7.17) Know how to determined electron pair geometry and molecular geometry (VSEPR model)

• (7.18) Know the definition of electronegativity

• (7.19) Know how to determine bond polarity and the definitions of covalent and polar covalent bonds

• (7.20) Know how to determine molecular polarity by molecular shape and bond polarity

Chp 8 - NOMENCLATURE

• first 36 elements (name, symbol, atomic number using periodic table)

• diatomic elements (name and symbol)

• anions (name, symbol and charge)

• cations (name, symbol and charge)

• nonmetal-nonmetal (covalent) compounds (symbol and name)

• metal-nonmetal (ionic or salt) compounds (symbol and name)

• acids (hydrogen – nonmetal compounds)

UNIT 3

Chp 9 – THE MOLE CONCEPT AND CHEMICAL FORMULAS

• (9.1) LAW OF DEFINITE (or CONSTANT) COMPOSITION – A compound is always made up of the same elements combined in a constant proportion by mass.

• (9.2 – 9.3) Molecular formulas and formula mass (amu)

• (9.4) Calculate and use percent composition of elements in compounds:

• (9.5 – 9.8) Mole – Avagadros number - molar mass (g)

• (9.10) Mole and chemical formulas

• (9.11) Conversions: mass -----> mole -----> molar mass

• (9.12) Calculations dealing with purity of samples

• (9.13 – 9.15) Empirical and molecular formulas

Chp 10 CHEMICAL CALCULATIONS INVOLVING CHEMICAL EQUATIONS

• (10.1) LAW OF CONSERVATION OF MASS – In a non-nuclear reaction, mass is constant, it is neither created nor destroyed.

• (10.2 - 10.4) Writing and balancing chemical equations

• (10.5) Know the different types of reactions (define, recognize, write chemical equations)

← synthesis (combination) reactions

← decomposition reactions

← single-replacement reactions (redox reactions)

← double-replacement precipitation reactions

← combustion (burning reactions)

← double-replacement neutralization reactions

• (10.6 – 10.7) Interpreting chemical equations ( conversion factors from chemical equations and the LAW OF CONSERVATION OF MASS

• (10.8) STOICHIOMETRY - Mass calculations involving chemical equations

• (10.9) Limiting reactants

• (10.10) Percent yield

UNIT 4

Chp 11 STATES OF MATTER

• (11.1 – 11.7) Know the differences between states and how the kinetic molecular theory applies.

• (11.8) Energy changes that occur when a substance changes state.

• (11.13 – 11.15) Evaporation, vapor pressure and boiling points of liquids

• (11.16) Know the different types of intermolecular forces (London forces – induced dipole, dipole-dipole, hydrogen bonding) and how the properties of liquids are affected by intermolecular forces

• (11.16) Water is a unique substance

Chp 13.1 – 13.4

• Characteristics of solutions:

← (13.1) terminology

← (13.2) factors affecting solubility

• (13.3 – 13.4) Know factors affecting solution formation (“like dissolves like”) and solubility rules

Chp 14.6 – 14.10

• Electrolytes and solution conductivity

• Solutions of ionic compounds

• Strong and weak acids

• Net ionic equations

• Single replacement reactions (redox reactions)

• Double replacement that form precipitates (double replacement reactions) and molecules (neutralization reactions)

• Double replacement that form unstable products

• Double replacement with undissolved reactants

Chp 13.5 – 13.11

• (13.5) Solution calculations:

← (13.6) percentage concentration by mass

← (13.7) ppm and ppb

← (13.8) calculation of molarity

• Stoichiometric solution calculations:

← (13.10) dilution calculations

← (13.11) yield calculations (theoretical yield. percent yield, limiting reactant), calculating molarity and (14.15) titration calculations

Chp 14 ACIDS AND BASES

• (14.1 – 14.2) Know the Arrhenius and Bronsted-Lowry definitions of acids and bases

• (14.3 – 14.4) Know how to identify acids and bases and conjugate acids and bases

• (14.5) Acid – base strength

• (14.11 – 14.12) Know water equilibrium, definition of pH and pOH and how to calculate pH and pOH.

PRECOURSE QUESTIONNAIRE

Name ________________________________________________________

Phone _________________________________________________________

Email _________________________________________________________

Year last chemistry course taken________________ Where taken?__________________________________

If taken at Solano, Course name________________________ Instructor______________________________

Major or career goal _______________________________________________________________________________

Why are you taking this course and what do you hope to accomplish in this course? ______________________________

_________________________________________________________________________________________________

_________________________________________________________________________________________________

_________________________________________________________________________________________________

_________________________________________________________________________________________________

What chemistry course (if any) do you plan to take next?____________________________________________________

What other science courses are you taking this semester?____________________________________________________

__________________________________________________________________________________________________

What college (if any) do you intend to transfer to finish your education?

_________________________________________________________________________________________________

Anything else I should know?_________________________________________________________________________

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